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Do elements in group 8 readily or rarely form ions?
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
What kind of bonds form when atoms steal electrons?
This is an ionic bond.
In terms of electrons in the periodic table why are group 1 metals very reactive and group 7 non-metals very reactive too?
Group 1 metals are very reactive because they have one electron in their outer shell, which they readily lose to achieve a stable electron configuration. Group 7 non-metals are very reactive because they are one electron short of a full outer shell, so they can easily accept an electron to achieve stability. This makes both group 1 metals and group 7 non-metals highly reactive in order to achieve a stable electron configuration.
Does the number of valence electrons in an atom of an element determines many properties of the element including the ways in which the atom can bond with other atoms?
Yes. The atom only bonds spontaneously if its to become more stable. So depending on the valence electrons, they have different forms of getting that stability. Let's see: Elements from the first and second group have 1 and 2 electrons of valence, respectively, so they tend to give them up. That's why they tend to bond with ionic bonds. They never steal electrons from others. Elements from the 17th group, are missing one electron to have their valence orbitals full, so again, they tend to steal electrons from those of group 1, forming stable ionic bonds. They can also give up some of their electrons, but more commonly they prefer to steal one. Elements like N and C, have their valence orbitals close to 50% filled, so they tend to prefer sharing electrons, that is, covalent bonds. Finally noble gases, have their valence orbitals filled with electrons, so they don't react with anything, and the only bonds they make, are weak Van der Waal bonds between themselves.
What are chemical bonds that steal electrons?
Chemical bonds that steal electrons are known as ionic bonds. In ionic bonding, one atom gives up electrons to another atom, resulting in the formation of positively and negatively charged ions that are held together by the attraction of opposite charges. This process typically occurs between a metal and a nonmetal.
Why do elements form ion?
Both of the elements will have two different electronegativities. When there is a large difference between the two electronegativities, one element will "steal" one or more electrons from the other element. The energy required for this is ionization energy, and increases as an element takes more electrons from another. My answer: Elements are stabilized when they contain a "complete shell" or the noble gas configuration of electrons, which is usually eight electrons. Elements that have a number of electrons close to that of a noble gas, will lose or gain electrons easily. For example, elements in the column just to the left of the noble gases have one fewer electron than the noble gas next to it, and therefore they tend to gain one electron easily. Elements in the column on the far left of the periodic table have one more electron than the noble gas in each row, and they tend to lose one electron easily. Because the protons contribute the positive charge, and the electrons contribute the negative charge, an ion is formed when an element gains or loses one or more electrons.
Do elements in group 8 readily or rarely form ions?
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
Why is it easy for oxygen to react with other elements?
Oxygen is a really strong oxidizing agent, meaning it's really greedy with electrons. It really wants to become stable like the noble gases, who have completely filled electron shells. The only way to get electrons is to oxidize other elements and steal their electrons. That's why oxygen is so reactive.
What will chlorine do to become more stable?
Chlorine achieves stability by gaining one electron to complete its outer shell, forming a chloride ion with a negative charge. Chlorine can also share electrons with other elements to achieve stability through covalent bonds.
What causes an element to be reactive?
An element's reactivity is influenced by its ability to gain or lose electrons to achieve a stable electron configuration. Elements with incomplete outer electron shells are generally more reactive as they can easily form bonds with other elements to gain stability. Reactivity can also be affected by factors such as atomic size and electronegativity.
What category of elements on the periofic table tends to create negatively charged ions?
Nonmetals tend to create negatively charged ions. This is because nonmetals have a higher electronegativity, meaning they have a greater tendency to gain electrons to achieve a stable electron configuration. This results in the formation of negatively charged ions, known as anions.
What compounds steal electrons?
DCPIP acts as an electron acceptor of a Hill Reacton. In this way, it "steals" electrons.
When P become a ion it becomes P3- not P5 why?
Phosphorus typically forms P3- ions because it gains three electrons to achieve a full outer shell of electrons, making it more stable. It is energetically more favorable for phosphorus to gain three electrons than to lose five electrons to achieve stability as P5-.
What kind of bonds form when atoms steal electrons?
This is an ionic bond.
Is a group in the periodic table more reactive near the top or the bottom?
A group in the periodic table is typically more reactive near the bottom. This is because elements in the same group have similar outer electron configurations, but as you move down a group, the atoms get larger, making it easier to lose or gain electrons, which can increase reactivity.
If you steal from a store are there cameras?
Yes most likely there will be.
In terms of electrons in the periodic table why are group 1 metals very reactive and group 7 non-metals very reactive too?
Group 1 metals are very reactive because they have one electron in their outer shell, which they readily lose to achieve a stable electron configuration. Group 7 non-metals are very reactive because they are one electron short of a full outer shell, so they can easily accept an electron to achieve stability. This makes both group 1 metals and group 7 non-metals highly reactive in order to achieve a stable electron configuration.
